Question

balance each half reaction assuming it's in a basic solution. please post the steps too!
CH_3OH(aq)->CH_2O(aq)

Answer 1

\[CH_3OH(aq)\rightarrow CH_2O(aq)\]

Answer 2

first determine what atom is being oxidized and what atom is being reduced.

Answer 3

i.e. assign oxidation states

Answer 4

I'm still confused because normally there are two reactants but here there is one and I don't know how to formulate the answer. Please help!

Answer 5

it think you may be missing \(H_2\) on the right side of the equation.

Answer 6

because, as i see it, only carbon is changing in oxidation state.

Answer 7

Here's the problem!

Answer 8

So, then does this mean that I only have to do one step right? How would I go about oxidizing the Carbon then?